The increase in positive charge increases the attraction between the nucleus and the electrons of the atom. As the number of protons increase, the nucleus of the atom becomes more positively charged. This is because the number of protons increase moving to the right of the row. When moving left to right across a period, the atomic size decreases. Going Left and Right Across Periods (Rows)
As a result, the electrons are not held as tightly towards the nucleus. In addition, the electron shells in between the valence shell and nucleus present electron shielding that also minimizes the attraction. Also, the new orbital is further away from the nucleus, meaning the attraction between the positively charged nucleus and the valence electrons decrease. This is because as you go down the period table, new valence shells are added and thus, increasing the radius. When moving down a group, the atomic size increases. The atomic size, or atomic radius, is the distance between the nucleus of an atom to the outermost electron orbital, where the valence electrons are. These patterns are called periodic trends. The tendencies of these patterns increase or decrease as you move along the columns and rows of the table. Specific patterns of certain elemental characteristics are present in the periodic table.
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